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# Why is the ha state function and q is not?

The state function is independent of the path to obtain specific values, such as energy, temperature, enthalpy, and entropy. Enthalpy is the amount of heat released or absorbed under constant pressure. **Heat is not a function of state as it simply transfers energy into or out of the system;** It depends on the pathway.

## Why is Q not a state function?

q is not a state function **Because it doesn’t just depend on the initial state and the final state**; The value of q depends on the path to the final q. Here is an example of why heat is not a state property: Consider raising the temperature of 50.0g of water from 25.0°C to 50.0°C.

## Why are work W and heat Q not state functions?

Temperature is a state function. …heat and work are not state functions.A job cannot be a state function **because it is proportional to the distance the object moves**which depends on the path used to get from the initial state to the final state.

## Why is Delta H not a state function?

ΔH is a function of two states, the initial state and the final state. For a given final state, there can be infinite values of ΔH, depending on the initial state.for **Given an initial state, there can be infinite** The ΔH value depends on the final state. Therefore, ΔH is not a state function.

## Why is the change in the state function not a state function?

We say that the change in the value of the state function depends only on the initial and final states of the system; the change in the value of the state function **Does not depend on the path in which the change occurs**.

## State Functions and Thermodynamics

**19 related questions found**

## Why is heat not a state function?

The state function is independent of the path to obtain specific values, such as energy, temperature, enthalpy, and entropy. Enthalpy is the amount of heat released or absorbed under constant pressure.Heat is not a state function **because it simply transfers energy into or out of the system;** It depends on the pathway.

## Which of the following is not a state function?

**Work** Not a state function as it depends on the path followed.

## Are U and H state functions?

Enthalpy is a state function because it is defined in terms of the state function. U, P, and V are all state functions. Their value depends only on the state of the system, not on the path to reach their value. … so, **H is the state function**.

## Is enthalpy reversible?

Therefore, the enthalpy change of an endothermic reaction is always positive. …whether the reaction is endothermic or exothermic depends on where it goes; **Some reactions are reversible**when you reduce products to reactants, the change in enthalpy is reversed.

## Is the enthalpy change a function of the path?

Enthalpy is **state function** Because it depends only on two thermodynamic properties of the current state of matter (like temperature and pressure, or temperature and entropy, or any pair of other state functions). It does not depend on the path that matter follows to get there.

## Is exotherm positive or negative?

A chemical reaction or physical change is exothermic if the system releases heat into the surrounding environment. Since the surrounding environment is gaining heat from the system, the temperature of the surrounding environment will increase.The symbol q for an exothermic process is **negative** Because the system is losing heat.

## Why is Q a path function?

Path functions and point functions are introduced to identify thermodynamic variables.path functions: their **The size depends on the path followed in the process and the final state**. Work (W), heat (Q) are path functions.

## Why is work not a thermodynamic property?

Work and heat are not thermodynamic properties, but process quantities: **Energy flow across system boundaries**A system contains no work but can do work, likewise, in formal thermodynamics a system contains no heat but can transfer heat.

## Is it a QW state function?

**Neither q nor w are state functions** But q+w is a state function.

## What is an example of a state function?

The others given in the exercises, i.e. internal energy, pressure, volume, temperature are all state functions.Examples of state functions include **(1) Internal Energy, (3) Volume, and (4) Pressure**. This is because the state function is a value that depends on a particular system state.

## Why is internal energy a state function and work is not?

Why is internal energy a function of state and not work? **The change in internal energy in the process depends only on the initial and final states, while the work depends on the path followed**. Therefore, internal energy is a function of state, but work is not.

## What is simple enthalpy?

enthalpy, **The sum of the internal energy of a thermodynamic system and the product of pressure and volume**. . . If the only work done is the volume change at constant pressure, then the enthalpy change is exactly equal to the heat transferred to the system.

## What does it mean when the enthalpy is zero?

temperature remains constant, so **energy change** zero (U=0). Therefore, the heat absorbed by the gas is equal to the work done by the ideal gas to its surroundings. The enthalpy change is also equal to zero because the energy change is zero and the pressure and volume are constant.

## Is the enthalpy change isothermally zero?

The change in enthalpy is **zero** Suitable for isothermal processes consisting only of ideal gases. For an ideal gas, enthalpy is only a function of temperature. By definition, an isothermal process is performed at a constant temperature. Therefore, in any isothermal process involving only ideal gases, the enthalpy becomes zero.

## What is the difference between a state function and a path function?

A state function is a property that describes a particular state, independent of the path taken to reach that state.In contrast, the function **value** Depending on the path obtained between two states is called a path function.

## Which quantity is not a state function?

Reply: **Work** is not a state function, as it does not depend on the path followed.

## What is the basis for the first law of thermodynamics?

The first law of thermodynamics is based on **Energy conservation law**which states that energy cannot be created or destroyed, but can be transferred from one form to another.

## Is enthalpy a state function or a path function?

As represented by the solution of the integral, the enthalpy is **state function** Because it depends only on initial and final conditions, not on the path that establishes those conditions. Therefore, the integral of the state function can only use two values: the final value and the initial value.

## Which of the following is not a state function? `?

**get the job done** is a path function (as it depends on a curve also called a path), it is not a thermodynamic state function. So the correct answer is option B, the job is done. Note: Zero Kelvin is called absolute temperature.

## Is the work done in an isothermal process a state function?

Because according to the first law of thermodynamics, the heat of constant volume is equal to the change of internal energy. So, it is also a state function. …as stated in the solution, the work done only in the isothermal process is path dependent, so **it is not a state function**.